Question

Antimony pentachloride, SbCl5, decomposes according to the following equation:
←
SbCl5(g) → SbCl3(g) +Cl(g)

An equilibrium mixture in a 5.00 L flask at 448 °C contains [SbCl5] = 0.002575 M, [SbCl3] = 0.008014 M and [Cl2] = 0.008011 M

1.State the type of equilibrium in the reaction

2.Calculate the mass in grams of each species that will be found when the mixture is transferred into a 2.00 L flask at the same temperature.

Answer 1

1.) chemical equilibrium is the state in which both reactants and products are present in concentration which have no further tendency to change with time

so lets calculate the value of equilibrium constant

K=$\dfrac{[SbCl_3][Cl_2]}{SbCl_5}=\dfrac{0.008014\times0.008011}{0.002575}=0.025$